This preview has intentionally blurred sections. Sign up to view the full version.
View Full DocumentThis preview has intentionally blurred sections. Sign up to view the full version.
View Full Document
Unformatted text preview: 1 CHM3400  Lecture 3 – Jan 10 Maxwell distribution laws and molecular collisions (Chapter 2 p. 2531) If we want to determine the velocity distribution for a large number of particles, we need to rely on a statistical treatment. The MaxwellBoltzmann distribution (based on classical statistical mechanics) gives a representation of the velocity distribution for an ensemble of particles. T k E B kin 2 3 = 2 2 1 v m In the previous lecture, we saw that the temperature of a gas is related to the average kinetic energy of the particles (rootmeansquare velocity ): 2 MaxwellBoltzmann distribution x B x B dv T k mv T k m N dN ⎟ ⎟ ⎠ ⎞ ⎜ ⎜ ⎝ ⎛ − ⎟ ⎟ ⎠ ⎞ ⎜ ⎜ ⎝ ⎛ = 2 exp 2 2 2 / 1 π Fraction of particles moving at velocity v x + d v x along direction x ⎟ ⎟ ⎠ ⎞ ⎜ ⎜ ⎝ ⎛ − ⎟ ⎟ ⎠ ⎞ ⎜ ⎜ ⎝ ⎛ = T k mc T k m c c f B B 2 exp 2 4 ) ( 2 2 / 3 2 π π Can rewrite this for the general velocity (directionless) c : Probability function (i.e., number/fraction of molecules) Velocity c Mass of particle Absolute temperature Velocity c 3 Understanding the MB function ⎟ ⎟ ⎠ ⎞ ⎜ ⎜ ⎝ ⎛ − ⎟ ⎟ ⎠ ⎞ ⎜ ⎜ ⎝ ⎛ = T k mc T k m c c f B B 2 exp 2 4 ) ( 2 2 / 3 2 π π N 2 @ 300 K 200 400 600...
View
Full
Document
This note was uploaded on 05/29/2011 for the course CHM 3400 taught by Professor Seabra during the Spring '08 term at University of Florida.
 Spring '08
 SEABRA
 Physical chemistry, Mole, pH

Click to edit the document details